Some Chemical Reactions in Everyday Life
Science being a subject of common interest, it is very intriguing to analyze
visual experiments happening in day-to-day life. There are a plethora of
products that you use everyday, which are formulated with application of
chemical reaction. Say for example; toothpaste, soap, shampoo, cleaning agent,
etc. are all results of chemical reactions. Following are some of the most
profound chemical reactions, which we encounter in everyday life :
Aerobic Respiration
Do you know indulging in physical movements is associated with a chemical reaction? The process requires energy, which is yielded by aerobic respiration. Over here, respiration helps breaks down glucose (an energy source) into water, carbon dioxide and energy in form of ATP (adenosine triphosphate). The balanced cellular respiration equation is represented as:
C6H12O6 + 6O2 → 6CO2+ 6H2O + Energy (36 ATPs)
Anaerobic Respiration
Due to overexercising, sometimes our body cells run out of oxygen and respire anaerobically. This cause synthesis of lactic acid and cause muscle cramps. Anaerobic respiration is observed in some bacteria, yeast and other organisms. In contrary to the aerobic type, it breaks down glucose in the absence of oxygen, resulting in production of ethanol, carbon dioxide and energy. Anaerobic respiration equation is:
C6H12O6 → 2C2H5OH + 2CO2 + Energy
Photosynthesis
Photosynthesis is the process by which green plants manufacture their own food. This occurs in presence of sunlight and other raw materials, namely carbon dioxide and water. The chlorophyll pigment harvests the light energy from sunlight, which is then converted into glucose by the phenomenon of photosynthesis. In short, it is the opposite of aerobic respiration. The equation for photosynthesis is:
6 CO2+ 6 H2O + Light energy → C6H12O6 + 6 O2
Rusting of Iron
Very often, you notice a coating of rust over unpainted iron surfaces, which gradually leads to disintegration of iron. This is nothing, but a chemical phenomenon called rusting. In this case, iron (a very reactive metal) combines with oxygen in presence of water (more precisely, atmospheric moisture), resulting in formation of iron oxides. The chemical reaction behind rusting can be simply represented as:
Fe + O2 + H2O → Fe2O3. XH2O
Propane Grill
Have you ever prepared meat in a propane grill? The meat placed over the burner is cooked with the help of heat energy released after burning of propane gas. Thus, propane is the reactant which when burnt with the help of oxygen gives heat energy and other byproducts. Check out the balanced equation for the combustion reaction that take place in a propane grill:
C3H8 + 5O2 → 4H2O + 3CO2 + energy
Whether you consider cooking, souring, fermenting or burning, there is a chemical reaction accompanying these everyday processes. Thus, it won't be wrong to say learning chemistry and chemical reactions start at home.
Aerobic Respiration
Do you know indulging in physical movements is associated with a chemical reaction? The process requires energy, which is yielded by aerobic respiration. Over here, respiration helps breaks down glucose (an energy source) into water, carbon dioxide and energy in form of ATP (adenosine triphosphate). The balanced cellular respiration equation is represented as:
C6H12O6 + 6O2 → 6CO2+ 6H2O + Energy (36 ATPs)
Anaerobic Respiration
Due to overexercising, sometimes our body cells run out of oxygen and respire anaerobically. This cause synthesis of lactic acid and cause muscle cramps. Anaerobic respiration is observed in some bacteria, yeast and other organisms. In contrary to the aerobic type, it breaks down glucose in the absence of oxygen, resulting in production of ethanol, carbon dioxide and energy. Anaerobic respiration equation is:
C6H12O6 → 2C2H5OH + 2CO2 + Energy
Photosynthesis
Photosynthesis is the process by which green plants manufacture their own food. This occurs in presence of sunlight and other raw materials, namely carbon dioxide and water. The chlorophyll pigment harvests the light energy from sunlight, which is then converted into glucose by the phenomenon of photosynthesis. In short, it is the opposite of aerobic respiration. The equation for photosynthesis is:
6 CO2+ 6 H2O + Light energy → C6H12O6 + 6 O2
Rusting of Iron
Very often, you notice a coating of rust over unpainted iron surfaces, which gradually leads to disintegration of iron. This is nothing, but a chemical phenomenon called rusting. In this case, iron (a very reactive metal) combines with oxygen in presence of water (more precisely, atmospheric moisture), resulting in formation of iron oxides. The chemical reaction behind rusting can be simply represented as:
Fe + O2 + H2O → Fe2O3. XH2O
Propane Grill
Have you ever prepared meat in a propane grill? The meat placed over the burner is cooked with the help of heat energy released after burning of propane gas. Thus, propane is the reactant which when burnt with the help of oxygen gives heat energy and other byproducts. Check out the balanced equation for the combustion reaction that take place in a propane grill:
C3H8 + 5O2 → 4H2O + 3CO2 + energy
Whether you consider cooking, souring, fermenting or burning, there is a chemical reaction accompanying these everyday processes. Thus, it won't be wrong to say learning chemistry and chemical reactions start at home.
Read more at Buzzle: http://www.buzzle.com/articles/chemical-reactions-in-everyday-life.html
What is the difference between aerobic and anaerobic respiration ?
BalasHapus1. Differences in Oxygen Requirement
HapusAs alluded to in the second sense, the difference between aerobic and anerobic respiration is either the presence or absence of an organism against the presence of oxygen in the respiratory process. In aerobic respiration, oxygen is needed because it is an important element that supports the success of catabolism. While in the process of aerobic respiration, organisms do not need to be noticed oxygen.
2. Location Differences
The aerobic and anaerobic respiratory processes also occur in different locations. Aerobic respiration occurs in organelles called mitochondria, while anaerobic respiration takes place in the cytoplasm.
3. Differences Process and Stages
Differences in aerobic and anaerobic respirations are also in the process and stages. The aerobic respiration process is more complicated and complex because it passes through stages such as glycolysis, the krebs cycle, and electron transport. While anaerobic respiration has a simple process, namely through the stage of glycolysis or fermentation.
4. Differences in Energy Products Generated
The aerobic respiration process will produce far greater energy of anaerobic respiration processes. Aerobic respiration generally produces energy of 36 ATP, while anaerobic respiration produces only energy from 2 ATP. Differences Butter and Margarine
5. Differences in Side Results
Aside from the energy products it produces, the aerobic and anaerobic respiration differences are also in the byproducts that are formed during the process. The aerobic respiration overhauls the substrate to completely carbon dioxide and air, all the hdrogens that are released from the substrate are in the process of burning with oxygen and generating air. Meanwhile, in the anaerobic respiration the substrate is overhauled into the air imperfectly. Examples of hydrogen detached from the substrate are being processed to rise to other forms and form various types of acids such as pyruvic acid, lactic acid. And ethanol.
What light energy is used in photosynthesis process?
BalasHapusUsually the light used in photosynthesis is sunlight, but artificial light like a lamp can be used as well, but not as good as sunlight
HapusIn what form plants produce food ?
BalasHapusthankyou badruzaman,nice question,Photosynthesis produces glucose, and oxygen so what form was that glucose? the answer is C6O6H12
HapusHow does aerobic breathing produce an energy?
BalasHapusAerobic respiration
HapusAerobic Respiration is a form of cellular respiration that requires oxygen to produce energy. Aerobic respiration is the process of generating energy by the full oxidation of nutrients through the Krebs cycle in which oxygen is the last electron acceptor. With aerobic respiration, glycolysis continues with the Krebs cycle and oxidative phosphorylation. Post-glycolytic reactions occur in the mitochondria in eukaryotic cells, and in the cytoplasm in prokaryotic cells. Aerobic metabolism is more efficient than anaerobic metabolism in terms of net gain of ATP.
The process of releasing energy works most efficiently if oxygen is used. Aerobic Respiration is a normal form of respiration. This requires oxygen and releases the most energy from glucose. When we breathe like this we inhale oxygen and emit carbon dioxide out. During aerobic respiration 1 mole of glucose produces 2,830 kilojoules of energy. Aerobic respiration produces energy, carbon dioxide and water. Aerobic respiration occurs within cells. All cells need energy supply to perform their functions. Food and oxygen are transported to cells in humans by blood in the circulatory system. Oxygen comes from the lungs of the respiratory system and the food comes from the small intestine of the digestive system. Cell mitochondria are the true location for aerobic respiration. When food is burned to release energy by using oxygen two waste products are produced: carbon dioxide and water. The aerobic respiration process can be represented by the word equation:
Food + oxygen -> energy + carbon dioxide + water
Aerobic respiration is the event of burning nutrients using oxygen from breathing to produce energy in the form of ATP. Furthermore, ATP is used to meet life processes that always require energy. Aerobic respiration is also called breathing, and occurs in the lungs. Meanwhile, at the cellular level of respiration occurs in mitochondrial organelles. The simple respiratory reaction is as follows:
C6H12O6 + 6O2 → 6 CO2 + 6H2O + 36 ATP
Aerobic respiration occurs gradually as for the stages:
A. Glycolysis
Glycolysis is a reshuffle of glucose into pyruvic acid in an anaerobic cytosol. There is enzymatic activity and involves the energy of ATP and ADP. The end result of glycolysis is 2 moles of pyruvic acid for every 1 mole of glucose, 2 moles of NADH as a source of high-energy electrons, 2 moles of ATP for every mole of glucose.
B. Daur Kreb`s
The occurrence of Ko-A assimilation with oxaloacetic acid (the change of acetyl Ko-A to CO2 with energy release), forming citric acid then this event is often called cycle of citric acid (tricarbosilic acid), occurs in mitochondrial matrix.
Each glucose molecule produces 2 molecules of asset coenzyme A and 4 molecules of CO2. High-energy electrons from glycolysis and Kreb's cycle are transferred to the electron-carrying chain.
Each glucose molecule produces 2 molecules of acetyl coenzyme A and 4 CO2 molecules, high-energy electrons from the glycolysis of the Kreb's cycle are transferred to the electron-carrying chain.
C. Electron Transfer
Occurs in the mitochondrial membrane, high-energy hydrogen reacts with oxygen (as the final acceptor) by the cytochrome enzyme, H2O is formed. Hydrogen from the Kreb cycle merged with FADH2 and NADH is converted to electrons and protons. In electron transfer 34 ATP is generated.
Please tell me why the iron can be rust?! And give me solution about it!m
BalasHapusProcess of Corrosion Occurrence
HapusA. The Process of Corrosion
Corrosion (Kennet and Chamberlain, 1991) is a decline in the quality of metals resulting from electro-chemical reactions to the environment. Corrosion or rusting is a chemical phenomenon in metallic materials which, in turn, represent the reaction of metals into ions on metal surfaces in direct contact with aqueous environments and oxygen. The most common example, is the iron metal with the formation of oxide rust. Thus, corrosion caused many losses.
Metal corrosion involves the anodic process, ie the oxidation of metals into ions by releasing electrons into the metal and cathodic processes which consume the electrons at the same rate: the cathodic process is usually the reduction of hydrogen ions or oxygen from the surrounding environment. For examples of corrosion of ferrous metals in humid air, for example, the reacting process can be expressed as follows:
Anode {Fe (s) → Fe2 + (aq) + 2 e}
X 2
Codes O2 (g) + 4H + (aq) + 4 e → 2 H2O (l)
+
Redox 2 Fe (s) + O2 (g) + 4 H + (aq) → 2 Fe2 ++ 2 H2O (l)
From the electrode potential data can be calculated that the standard for this corrosion process, ie E0 = + 1.67 V; This reaction occurs in the acidic environment wherein H + is partially obtainable from the reaction of atmospheric carbon dioxide with water forming H2CO3. The Fe + 2 ion formed, in the anode is further oxidized by oxygen to form iron (III) oxide:
4 Fe + 2 (aq) + O2 (g) + (4 + 2x) H2O (l) → 2 Fe2O3x H2O + 8 H + (aq)
This iron hydrate (III) oxide is known as iron rust. Electrical circuits are referred to by the migration of electrons and ions, which is why rapid corrosion occurs in salt water.
If corrosion processes occur in an alkaline environment, then the cathodic reaction is
Occurs, namely:
O2 (g) + 2 H2O (l) + 4e → 4 OH- (aq)
Further oxidation of Fe2 + ions does not take place because of the slow motion of the ions so that it is difficult to relate to the oxygen of the outside air, in addition to the ions being instantly captured by the hexasianoferic (II) complex salt to form a stable stable blue art. The alkaline environment is available due to the complex of potassium oxoanoate (III).
Real-time corrosion of iron rapidly occurs and continues, because the iron layer (III) oxide that occurs porous so easily penetrated by air or water. But although aluminum has a much more negative negative reduction potential than iron, but the corrosion process continues to be inadequate because of the oxidation of Al2O3, the coating is not porous to protect the coated metal from contact with the outside air.
B. The Impact Of Corrosion
Karatan is a term given by society to the metal
Suffered porous damage. While the metal part is broken
And brownish-black in steel is called Rust. Theoretically rust is a term given to one type of metal only steel, while in general the term rust is more accurately called corrosion. Corrosion is defined as the degradation of the material (especially the metal and its alloys) or its nature by interacting with its environment.
Corrosion is an electrochemical process or reaction that is natural and continuous by itself, therefore corrosion can not be prevented or stopped completely. Corrosion can only be controlled or slowed down so that it slows down the process of destruction.
Viewed from the electrochemical aspect, corrosion is the process of transferelektron from metal to the environment. The metal acts as a cell providing an electron (anode) and its environment as an electron (cathode) receiver. The reaction that occurs in corrosive metals is oxidation, in which metal atoms dissolve into their environment by releasing electrons in the metal. As for the cathode reaction occurs, where the ions from the environment approach the metal and capture the electrons-
Electrons left on the metal.
How to prevent corrosion in iron can be done as follows:
HapusA. Painting
The function of painting is to protect the contact iron with water and air. Paints that contain lead and zinc will better protect the iron against corrosion. Painting should be perfect because if there is a part that is not covered by paint, then the iron under the paint will be corroded. Fences of buildings and bridges are usually protected from corrosion by painting.
B. Wrapped in plastic
Plastics prevent the iron from contact with water and air. Household appliances are usually wrapped in plastic to avoid corrosion.
C. Coating with chrome (Cromium plating)
Chrome gives a protective coating, so the chrome iron will become shiny. Cromium plating is done by electrolysis process. Chrome can provide protection even if the chrome layer is damaged. This method is generally done on motor vehicles, such as car bumpers.
D. Coating with tin (Tin plating)
Lead includes stainless metal. Tin packs of iron are generally coated with tin. Coating process is done electrolysis or electroplating. The tin layer will protect the iron as long as the coating is intact. If there is a scratch, the tin precisely accelerates the corrosion process because the iron electrode potential is more positive than tin.
E. Zinc coating (Galvanization)
Zinc can protect the iron even if the lining is damaged. This is because the iron electrode potential is more negative than zinc, so the iron in contact with the zinc will form an electrochemical cell with iron as a cathode. So the zinc will experience oxidation, while the iron will be protected.
F. Anode sacrifice (Sacrificial Anode)
Repairing corroded underground pipes may require costly repairs. This can be solved by sacrificial anode technique, that is by implanting the magnesium metal then connected to the iron pipe through a wire. The magnesium metal will rust, while the iron is not because magnesium is an active metal (easier to rust).